Copper exhibits only $+2$ oxidation state in its stable compounds. Why?
- ACopper is a transition metal in the $+2$ state.
- BThe high hydration enthalpy of $Cu^{2+}(aq)$ compensates for the second ionization enthalpy of Copper.
- CThe electron configuration of Copper in the $+2$ state is $[Ar] 3d^9 4s^0$.
- DCopper forms coloured compounds in the $+2$ state.
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| $(1) \ Cu$ | $(A) 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^{10}$ |
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| $(E) 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^3$ |
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